Which provides the greatest increase in entropy for a mole of substance?
a)Water melts at 0°C.
b)Liquid water is heated from 0°C to 25°C.
c)Gaseous water is converted to solid ice at 0.1°C.
d)Water is converted from liquid to vapor at 100°C.
e)Cannot be determined.
To determine which option provides the greatest increase in entropy for a mole of substance, we need to understand the concept of entropy and how it changes during phase transitions and temperature changes.
Entropy is a measure of the disorder or randomness of a system. It can be viewed as a measure of the number of ways particles can arrange themselves in a given system. In general, the transition from solid to liquid to gas increases the entropy, as the freedom of movement and disorder among particles increases.
Now, let's analyze each option:
a) Water melts at 0°C: This is the transition from solid ice to liquid water. During this process, the water molecules gain freedom of movement and are able to flow, increasing the entropy.
b) Liquid water is heated from 0°C to 25°C: This is a temperature change in the liquid phase. The increase in temperature adds energy to the water molecules, increasing their vibrational and rotational motions, which also increases the entropy, although to a lesser extent compared to a phase transition.
c) Gaseous water is converted to solid ice at 0.1°C: This is the transition from gas to solid. The water vapor molecules lose their freedom of movement and become fixed in a crystal lattice, decreasing the entropy.
d) Water is converted from liquid to vapor at 100°C: This is the transition from liquid to gas. During vaporization, water molecules gain even more freedom of movement, increasing the entropy significantly.
Based on the explanations above, we can conclude that option (d) provides the greatest increase in entropy for a mole of substance, as it involves the phase transition from liquid to gas. Therefore, the correct answer is option (d).
To determine which option provides the greatest increase in entropy for a mole of substance, we need to consider the phase transitions and temperature changes involved.
Entropy generally increases with an increase in temperature and with a transition to a more disordered state. So, let's consider the options:
a) Water melting at 0°C: This is a transition from a solid to a liquid state. Entropy increases due to the increased molecular motion and freedom. However, compared to other options, this transition has a relatively small impact on entropy.
b) Liquid water heated from 0°C to 25°C: This is a temperature increase without a phase transition. The increase in entropy is comparatively smaller than other options since the molecules are already in a liquid state.
c) Gaseous water converted to solid ice at 0.1°C: This is a transition from a gas to a solid state. Entropy decreases in this transition since the molecules become more ordered and have less freedom of motion.
d) Water converted from liquid to vapor at 100°C: This is a transition from a liquid to a gas state. This transition provides a significant increase in entropy as the molecules become more disordered and have more freedom of motion.
Based on the analysis above, option d) provides the greatest increase in entropy for a mole of substance.